To use molar mass values and a balanced chemical equation to relate the mass of reactants to the mass of products. Most problems include some additional conversions beyond the three stoichiometry steps. Includes 6 problems.
Mr. Glynch has three jumbo-sized test tubes that he is using to demonstrate the effect of reactant mass on the amount of product. Each test tube is half-filled with hydrochloric acid (HCl). He adds a known mass of mossy zinc to each test tube and quickly caps the top with a balloon to trap the gas that is produced. The reaction that occurs is ...
Zn(s) + 2 HCl(aq) → H2(g) + ZnCl2(aq)
The amount of zinc added to each test tube is:
Test Tube A: 2.20 g
Test Tube B: 4.40 g
Test Tube C: 6.60 g
The density of the hydrogen gas is 0.0905 g/L.
Use stoichiometry and conversion factors to determine the volume (in mL) of hydrogen gas produced in Test Tube A.
Volume of H2
mL
Determine the volume (in mL) of hydrogen gas produced in Test Tube B.
Determine the volume (in mL) of hydrogen gas produced in Test Tube C.
These results show that when the mass of Zn is doubled, the volume of H2 gas produced _______.
These results show that when the mass of Zn is tripled, the volume of H2 gas produced _______.
Some brands of antacid tablets contain aluminum hydoxide. The aluminum hydroxide has the ability to neutralize the excess stomach acid that can lead to indigestion. The balanced chemical equation for the neutralization of hydrochloric acid is shown below.
Al(OH)3(s) + 3 HCl(aq) → AlCl3(aq) + 3 H2O(l)
How many grams of hydrochloric acid (HCl) can be neutralized by 55.0 mg of aluminum hydroxide?
Mass of HCl
g
Many 4th of July firework displays used a reactant mixture known as flash powder that burns quickly and produces a loud noise upon ignition. The mixture consists of an oxidizer such as potatssium perchlorate and a metal such as aluminum. A common chemical reaction is
3 KClO4 + 8 Al → 3 KCl + 4 Al2O3
Suppose that a flash powder mixture contains 38.8 g of aluminum. What mass of potassium perchlorate will react with this aluminum?
Mass of KClO4
What mass of aluminum oxide will be produce by the reaction of 38.8 g of aluminum?
Mass of Al2O3
b
Gas burners burn methane (CH4) according to the reaction …
CH4 + 2 O2 → CO2 + 2 H2O
The methane is delivered through pipes. But the oxygen is provided by the air surrounding the stove top. Suppose a typical meal prep uses 7.40 g of methane.
What volume (in mL) of oxygen gas is removed from the air when burning this amount of methane? Assume a density of 1.43 g/L for oxygen gas.
Volume of O2
What volume (in mL) of carbon dioxide gas is released to the air when burning this amount of methane? Assume a density of 1.96 g/L for carbon dioxide gas.
Volume of CO2
The reaction below is one of relatively few reactions that takes place directly between two solids at room temperature. In this equation, the •8H2O in Ba(OH)2•8H2O indicates the presence of eight water molecules. This compound is called barium hydroxide octahydrate.
Ba(OH)2•8 H2O(s) + 2 NH4SCN(s) → Ba(SCN)2(s) + 10 H2O(l) + 2 NH3(g)
What mass of ammonium thiocyanate (NH4SCN) must be used if it is to react completely with 4.29 g barium hydroxide octahydrate?
Mass of NH4SCN
Thermite is a generic name given to a pyrotechnic mixture containing a metal powder and a metal oxide. When ignited, the components of the mixture react with each other and emits a spectacular amount of heat and light energy. The most popular of such reactions is …
Fe2O3(s) + 2 Al(s) → 2 Fe(l) + Al2O3(s)
What mass of iron(III) oxide must be used to produce 41.5 g iron?
Mass of Fe2O3
What mass of aluminum must be used to produce 41.5 g iron?
Mass of Al
What is the mass of aluminum oxide that is produced in this reaction?